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Q: . Commonly used standards for the direct determination of the normality of an acid. 2. It is used…
A: Given: 1. Commonly used standards for the direct determination of the normality of an acid. 2. It…
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A: Case 1: Concentration of weak acid and conjugate base are as follows: [CH3COOH] = 0.25 M [CH3COONa]…
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A: Given :- Kw at 10°C = 2.9 × 10-15 To be calculated :- pH of pure water at 10°C
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A: Reaction: H2Ox + OH- —->HOx- + H2OHOx- + OH- ——->Ox- + H2O Equilibrium: H2Ox ——>HOx- + H…
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Q: et ine the pH Of the Soluti quivalence point.
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Q: [ОН ] pH pH pH Calculated раper meter pH 1. 0.1 M 2. 0.01 M 3. 0.001 M 4. 0.0001 M [H,O° ] pH pH…
A: Given that : We have to calculate the pH for the given concentrations of [H3O+] and [OH-] ions.
Q: The acid dissociation constant K, of acetic acid (HCH, CO,) is 1.8 × 10¯°. Calculate the pH of a 2.3…
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Q: If a buffer solution is 0.260 M in a weak acid (K, = 5.3 × 10-5) and 0.470 M in its conjugate base,…
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Q: Which type of graph (log or linear) allows you to visually quantitate the differences in…
A: The graph that satisfies the straight line equation of the form y=mx+c are called linear graphs.…
Q: A solution is prepared at 25 °C that is initially 0.30 M in benzoic acid (HC,H,Co,), a weak acid…
A: Step 1: The given solution is a buffer of weak acid and its conjugate base. So, the Handerson…
Q: What is the concentration of hydroxide ions in pure water at 30.0∘C, if Kw at this temperature is…
A: The ionization of water is represented as,
Q: A solution of 0.05 M benzoic acid (C6H5COOH) and 0.10 M sodium benzoate (C6H5COONa) has a pH of 4.50…
A: The above-given problem can be solved using the Henderson-Hesselbalch equation. pH = pKa +…
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A:
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![What is the carbonate [CO3 4] concentration
for a system at pH = 10.9 and a total dissolved
carbonate concentration of 10-2.5 M?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e8b9c67-63da-4856-8557-a4b1bba4357d%2F8b491fd8-de6f-4bab-a407-46dac99fb206%2Fpwzef2l_processed.jpeg&w=3840&q=75)
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- Calculate the amount of 0.300M H2SO4 required to neutralize a 0.600g sample that is 50% FeO.4. (a) Calculate [H3O*] and [OH] for the solutions indicated: lemon juice, pH = 2.42 (1) (ii) household ammonia pH = 11.21 (iii) (iv) (v) phosphate buffer pH = 6.96 human urine pOH = 7.8 tomato juice pOH = 9.9What is the concentration of C6H5OHCOOH in a 0.1185 M C6H5OHCOONa? Answers are expressed in molarity. Ka for C6H5OHCOOH is 1.05e-3.
- Salt of anion X gives colorless gas when reacts with dil. HCl acid and can removes the color of potassium permanganate, salt X represents a) K2CO3 b) KCI c) KNO2 d) KNO34. What is the equilibrium concentration of PO4³ in a 0.351 M solution of H₂PO4(aq)? (K₁1 = 7.5 × 103, K₂2-6.2 × 108, K₂=4.8 × 10-13) 01) 62×108 M O2 48×10?M O 3) 15×10 4 M O4) 41×107 M 05) 48 × 10-¹3 MHNO3 is Available at a concentration of 18M. What Volume would you need in mL to obtain 0.250mol?
- H2AO4 is a weak acid. What is [AO42 in a 0.30 M H2AO4 solution? [Ka1 = 6.2 x 10-; Ka2 = 5.2 x 10-10 OA21 x 10-5 M OB 5.2 x 10-7 M OC0.60 M OD 6.2 x 10-7 M OE 0.30 M OF 6.2 x 10-10 M OG5.2 x 10-10 MWhich of the following compounds precipitates from a solution that has the concentrations indicated? (a) KClO4: [K+] = 0.01 M, [ClO4-] = 0.01 M (b) K2PtCl6: [K+] = 0.01 M, [PtCl62-] = 0.01 M (c) PbI2: [Pb2+] = 0.003 M, [I–] = 1.3 x 10–3 M (d) Ag2S: [Ag+] = 1 x 10–10 M, [S2–] = 1 x 10–13 MThe pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated?
- 7. barium hydroxide reacts with acetic acid: a. Write the balanced chemical equation: (PA6 + (po moitopo olussioM 18 1svlia + muiesngom A b. How many mL of 0.1 M Ba(OH)2 will be required to neutralize 20.0 mL of 0.25 M HC2H3O2? Horl noitabixo soitaosy tail noitub 19 jWhat is the concentration of CuS in a solution in which [H3O*] is held constant at 2.0x10 M?Considering 0.1 M acqueous solutions of each of the following, which solution hasthe lowest pH?(A) Na2CO3 (B) Na3PO4 (C) Na2S (D) NaCl(E) CH3COONa